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CHEM191 > Aqueous solutions > Flashcards

Aqueous solutions Flashcards

1
Q

The solubility of substances in aqueous biological solutions is crucial in which 3 processes?

A

Transport of gases
Transport of inorganic materials
Application and transport of drugs

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2
Q

Property that all atoms have to do with how much that atom wants to pull electrons towards itself away from other atoms that are attatched to it in the molecule

A

Electronegativity

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3
Q

When oxygen and hydrogen bonds have different electronegativities this is called what?

A

Polarbonds

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4
Q

A bond that has a delta positive and a delta negative end

A

Polar bond

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5
Q

A bond that doesn’t have partial changes due to the 2 atoms in the bond not having different electronegativities

A

Non polar bond

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6
Q

The most electronegative element in the periodic table

A

Fluorine

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7
Q

The water molecule is described as

A

Bent

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8
Q

Type of dipole-dipole interaction that you only get when you have polar bonds that contain OH, NH, or FH

A

Hydrogen bonding

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9
Q

Which 3 things does there need to be to get hydrogen bonding?

A

OH, FH, NH

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10
Q

Hydrogen bonding has important impacts on the …… of the molecule

A

Properties

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11
Q

The stronger the interactions between the molecules, the …… the boiling point will be because the ….. it will be to pull those molecules apart from each other

A

Higher
Harder

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12
Q

What gives a molecule a higher boiling point?

A

Strong interactions

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13
Q

Simplest molecule to exist that is liquid at room temp and atmospheric pressure

A

Water

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14
Q

Simplest molecule that could be the solvent for a biological system to evolve in

A

Water

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15
Q

Molecules are always moving around, hydrogen bonds are fixed and broken and are always moving around and never fixed in pairs

A

Liquid water

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16
Q

Molecules stop moving, hydrogen bonding is fixed between pairs of molecules

A

Solid

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17
Q

Why is solid water less dense than liquid water?

A

Because the molecules are further apart, and there is more space in between them

18
Q

At which degrees celcius does water maximum density occur?

A

4

19
Q

The freezing point of water ….. as pressure increases

A

Decreases

20
Q

Substances that give ions when dissolved

A

Electrolytes

21
Q

Explain how water is a solvent to sodium chloride

A

Water comes in and takes a chloride and surrounds it with water molecules and surrounds the negatively charged an ion with water molecules, so the postively charged end of the water molecules are closest to the negative charge on the an ion

22
Q

Why are some salts more difficult to dissolve in water than other?

A

Some dont mind being surrounded by water molecules, but some prefer to stay in the solid with their other cat ions and an ions

23
Q

Hydration spheres

A

Spheres of water molecules that surround the cations and the anions

24
Q

Explain why solubility is much less for gases eg oxygen than polar things

A

These interactions are much more weaker as we are having to induce a dipole in the O2 molecule rather than it being there all the time

25
Q

Formed when 1 or more chemical species dissolve in a liquid

A

Solution

26
Q

Substance that dissolves in a liquid. Can be solid, liquid or gas

A

Solute

27
Q

Liquid in which the solute dissolves

A

Solvent

28
Q

Dissolves to give ions in solution

A

Electrolyte

29
Q

Dissolves without the formation of ions

A

Non electrolyte

30
Q

When the amount of solute is much less than the amount of the solvent

A

Dilute solution

31
Q

When a solid dissolves, and the only thing you get in. the solution is cations and anions, its means it is a…..

A

Strong electrolyte

32
Q

When you put it in water, it can dissolve to give cations and anions but it doesnt have to

A

Weak electrolyte

33
Q

Explain why acetic acid isnt a strong electrolyte

A

Because most of the acetic acid molecules dissolve in water, and only some of them go onto give cations and anions, so therefore the dissolving process does not exclusively give cations and anions

34
Q

Water is a good solvent for many compounds because of its…

A

Polar nature

35
Q

Explain how OH bonds are polar

A

Due to the O being much more electronegative than the H, giving the O a partial negative charge and the H a partial positive charge

36
Q

When a polar molecule dissolves, what interaction drives the process?

A

A dipole-dipole interaction

37
Q

When a gas dissolves in water, what interaction drives this process?

A

Dipole-induced interactions

38
Q

A solid that dissolves in water to give ions

A

Electrolyte

39
Q

A strong electrolyte is one which…

A

Completely dissolves

40
Q

A weak electrolyte is one which…

A

Partially dissolves, giving an equilibrium between undissolved solid and dissolved ions

41
Q
A

CHEM191 (14 decks)

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